Acid base Definition and 46 Threads

I tried to solve the problem (problem 1 on this problem set) by noting that titrating to the equivalence point means neutralizing all of the NaOH with the titrant HCl. Since 15.4mL of HCl at 1.0M was used, then 0.00154 mol of HCl was used to neutralize the same amount of NaOH. Therefore, in...

The reason is that at the stoichiometric point the entirety of the analyte has been neutralized and the solution contains only the salt from the neutralization plus the ions from water autoprotolysis. The salt comes from the conjugate acid of the strong base and the conjugate base of the strong...

We start with 25ml of a 0.100M solution of ##\mathrm{HCOOH(aq)}## and as titrant we use a 0.150M solution of ##\mathrm{NaOH(aq)}##. For reference, we can calculate the initial pH of the formic acid solution, which comes out to 2.37. I will go over just the results of the initial calculations...

Here is an example Let me go through the concepts here. The stoichiometric point occurs when the number of moles of acid and base have the same ratio as present in the chemical equation. In the equation shown above, this is a 1:1 relationship. Acetic acid is a weak acid and at the...

This is all fine, but then there is the following I am under the impression that if an acid is weak (ie, only a small fraction of the molecules donate protons) then the conjugate base is strong (a large fraction of the molecules accept protons). But the snippet above seems to say that that...

I'd like to go through the steps in this calculation carefully to make sure I fully understand what is happening. We start with a total of three chemical compounds: ##\mathrm{H_2O, CH_3COOH}## and ##\mathrm{NaCH_3CO_2}## at ##\mathrm{25^\circ C}##. That is, we have water, a weak acid, and a...

##\mathrm{OH^-}## participates in the autoprotolysis of water. $$\mathrm{2H_2O(l)\rightleftharpoons H_3O^+(aq)+OH^-(aq)}$$ Now, the definition of a Bronsted-Lowry base is a compound that is a proton acceptor. ##\mathrm{OH^-}## accepts a proton and is thus a Bronsted-Lowry base. So, why do we...

I find the one (4s) + 3(4p) + 2(d) incorrect according to my knowledge.

First so that you can have some background I'd like to share an excerpt from the online lecture I'm studying. Here's a sample: "1880-Arrhenius defines an acid as a substance that , when dissolved in water, produces an increased concentration of hydrogen ions. 1900-Naunyn combines Arrhenius'...

The following are my works for the problems: I put squares on my final answers! Thank you!

Homework Statement Calculate the pH of the following solutions: (caution: these are hydrolysis reactions) a. an 0.30 M solution of NaF Homework Equations I think by hydrolysis reactions they mean that each of the given compounds is combined with $H_2O$. Then for a) NaF + HF <-->...

Homework Statement Calculate the pH of a 0.20 M solution of iodic acid ##(HIO_3)##. ##K_a## for iodic acid is 0.17 Homework Equations ##K_a = \frac{[H^+][IO_3^-]}{[HIO_3]}## The Attempt at a Solution ##[HIO_3] = 0.20## M. The concentration of ##[H^+]## and ##[IO_3^-]## should be the same...

Hi everyone. I was testing the pH of water that had alka seltzer placed in it. I used Bromothymol blue indicator to see the pH. The color changed to yellow, which suggests that the water was now acidic. I assume this is because of the CO2 bubbles that form which can acidify the H2O. Am I...

I tried looking for my unknown (209.70 g/mol) online and couldn't find it. The closest I found were H4O7V2(217.907 g/mol) and HCl2I(198.819 g/mol), but I know I am correct to a 2.7% accuracy. What other lists can I use to solve this?

Hi I am new to the concept of neutralization. My teacher told me that acids do not react with neutral salts. I want to know why not. If both are dissolved in water and both completely dissociate, why can't the ions of acid and salt exchange and perform a double displacement reaction. Moreover I...

I was thinking of a hypothetical waste system that uses nanotechnology to its advantage. At the individual level, waste just passes through into pipes when flushed like it normally does. But once it reaches the water treatment plant there is an initial filter to catch solid waste(in other...

Homework Statement To unclog a drain you add 26g of sodium hydroxide to 150mL of water. Calculate the pH and pOH for the solution you prepared. Can someone tell me if I'm doing it right. Homework EquationsThe Attempt at a Solution n = m/M n = 26/40 n = 0.65mol for 0.15L Does this mean that I...

Do pH and pKa refer to the same concept? The same question for pOH and pKb also. What does kWh actually mean. In have read that it is the ionic product and is the product of [H+] and [OH-] but what does it indicate. Does it have any full form?

Since Acetic Acid is a weak acid, it has a low Ka which means that the forward reaction is not favored as much as the reverse reaction. However, the Kb is even lower than the Ka...how is this possible? Shouldn't the Kb be higher to indicate that the reverse reaction is favored?

Homework Statement Student mix four reagents together, thinking the solutions will neutralize each other. The solutions mixed together are 50.0mL of .1 M HCl, 100mL of .2 M of HNO3, 500mL of .01 M CaOH, 200mL of .1 M RbOH. Did the acids and bases exactly neutralize each other? If not, calculate...

I'm having a lot of trouble predicting which compounds would be extracted into which layer (organic vs. aqueous) using acids and bases. Using the solvents dichloromethane (which would form the organic layer) and sodium hydroxide (would form the aqueous layer along with water), I am asked to...

Homework Statement In which one of the following solutions is silver chloride the most soluble? A) 0.181 M HCl B) 0.0176 M NH3 C) 0.744 M LiNO3 D) pure water E) 0.181 M NaCl Homework Equations the Ksp expression for the dissolution of AgCl is: Ksp = [Ag+][Cl-]The Attempt at a Solution...

Homework Statement I found this problem online for extra practice for my AP Chem class. https://www.quia.com/files/quia/users/jpugteach/APChem/AP-Chem-Chapter-19-Graphs.pdf The problem in question is number 4. I do not understand how to solve it and why the answer D is correct. Homework...

Homework Statement Methyl red has the following structure [not listed here on this post] Ka = 5.0 * 10 E -5 It undergoes a color change from red to yellow as a solution gets more basic. Calculate an approximate pH range for which the methyl red is useful. What is the color change and the...

Homework Statement [/B] NH3(aq) is a weak base with Kb = 1.8*10-5, Calculate [OH-] in a solution that is made by mixing togeather 500ml of 0.20M NH3(aq) and 500ml of 0.20M NH4CL(aq), what is the value of Ph?Homework Equations Henderson Hasselbalch: ph = Pka + log([conj.base/acid]) As well as...

Hey all! I have a silly doubt In acids and bases As you guys know The concentration of H+ ions For a weak acid Which does not undergo Complete dissociation Is given by mod H+=square root of Ka times C Where C is the initial concentration Of the acid And k is the ionization constant In the same...

Hi guys, my name is ferdinand. I'm curious about HSAB, especially to predict where the reaction goes. Exp: HI + NaF >>> HF + NaI H is hard acid I IS soft base Na is hard acid F is hard base, and HF Is hard.hard NaI Is hard soft. The reaction will goes to right or left? And why? And since hard...

what theories out of the major two ( Bronsted-Lowry Theory of acids and bases and The Lewis Theory of acids and bases) should we use in common problems, and which one is more reliable ?

i am doing my lab report and i just want to know how to calculate the absolute error of the acidic concentration and thank you.

Homework Statement the question asks to determine if the equilibrium is greater, equal or less than 1. one of the equation is the following: [CuI4]2- (aq) + [CuCl4]3- (aq) ↔ [CuCl4]2-(aq) + [CuI4]3- (aq) Homework Equations The Attempt at a Solution the solution given was...

Homework Statement Assuming stomach acid is 0.1 M HCl(aq), what volume of stomach acid can be neutralized by one antacid tablet? We have the titration curve we got with .5M HCl titrating a tablet dissolved in 100ml distilled water Homework Equations ? The Attempt at a Solution ?

Homework Statement 1.5000 g of diprotic weak acid H2A was dissolved in 100.00 mL volumetric flask. 25.00 mL aliqouts of this solution was titrated with a monoprotic strong base NaOH (0.08000 M). The titre volume of NaOH was 40.00 mL. Calculate the molecular weight of H2A. Homework...

Homework Statement Hi. I'm reaady to panic right now so if anyone could please take the time to answer my question I would HUGELY appreciate it! I seriously need to get this done soon as I also have a test tomorrow and i just want to cry because I'm getting nowhere... We did a lab...

Homework Statement after titrating sodium hydroxide with hydrofluoric acid, a chemist determined that the reaction had formed an aqueous solution of 0.020 mol/l sodium fluoride. determine ph of the solution Homework Equations The Attempt at a Solution Ka of HF= 6.3X10^-4 NaOH +...

Hi. In class, i am required to perform a titration where i am given a solution of sodium carbonate and a solution of hydrochloric acid of known concentration. I am to use the acid to calculate the percentage purity of the sodium carbonate. Im not really sure how to go about doing this. The...

Homework Statement Do not understand the question. 2. My Lab Results Topic : Volumetric analysis - Acid base purpose : To determine the exact concentration of a mineral acid, HXO4, and to determine the relative atomic mass of the element X. Materials : KA1 is a mineral acid, HXO4...

Hello everybody, I'm having difficulty understanding the rationalization behind the strengths of Bronstend Lowry acids and bases and my textbook isn't too helpful. Can someone please expalin to me: (1) What exactly is effective negative charge density? (2) how does electronegativiy correspond to...

Homework Statement Given H2SO4 + 2LiOH --> Li2SO4 + 2H2O, how many mL of a 0.700-M solution of KOH are needed to react with 235 mL of a 0.350-M H2SO4 solution? The Attempt at a Solution Really, I have none. My problem is that I don't understand what the question is asking. I could...

Homework Statement You dissolve an unknown quantity of weak acid HA into 50 mL of water. It only takes 1 mL of 5 M NaOH to completely neutralize the acid. The Ka of the acid is 3.2 x10^-4. What is the pH at the endpoint?Homework Equations Ka * Kb = Kw pH + pOH = 14 p(of whatever) = -log(of...

Homework Statement A vessel contains 500mL of .1 molar H2S solution. For H2S Ka1 = 1 x 10^-7 Ka2 = 1.3 x 10^-13. What will the pH be when 800mL of .1molar NaOH has been added. Homework Equations ph = -log([H]) ph = pka + log(B/A)The Attempt at a Solution This is how I started, I found the...

I tried looking for this online, but didn't really find anything can someone help me out I need an example of a naturally- occurring acid-base buffering system in an organism

I have a question concering acid base reactions. All strong acid-strong base reactions produce a water soluble salt and water with the exception of what? I need to know that along with the formula unit, total ionic and net ionic equation. Please any help would be appreciated. Thank you

Hi. I am having trouble with acid-base titration excercises. 0.02 L butanoic acid @ 0.1 M is titrated with 0.01 L NaOH solution @ 0.1 M. The Ka of butanoic acid is 1.54X10^-5. Find the pH. The answer is 4.81. I know how to find the pH when no NaOH is added, but I really don't see how the...

How many moles of H3O+ must be added to one liter of a solution to adjust the pH from 7.17 to 5.85? Correct answer 1.34E-6 (1.34 * 10-6) The correct answer is given, however I would like to know how to do this problem.

consider the titration of 50.0mL of 0.10 M methyl ammonia with 0.10 M HCl. Calculate the pH after 15mL of titrant= 11.05 25mL of titrant= 10.68 50mL of titrant= 8.98 60mL of titrant= ? At 60 mL there is an excess of 1 mmol of HCl. At this point do I say that the pH is 1 (-log of 0.10)...

I have several questions. 1.)Supose [H+] is 100 times less than the ka for an acidic acid-base indicator (see Eq.2), and enough acid is added to the the solution to raise [H+] by a factor of 10,000. What value did the ration of the different colored forms of the indicator, [ln-]/[H ln], have...